(A) Elevation in boiling point is given by $\Delta T_{b} = i \times K_{b} \times m$. For $NaCl$ $(58.4 \ g \approx 1 \text{ mole})$, $i = 2$. For gluc

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$NaCl$ solution will show higher elevation of boiling point

(A) Elevation in boiling point is given by $\Delta T_{b} = i \times K_{b} \times m$. For $NaCl$ $(58.4 \ g \approx 1 \text{ mole})$, $i = 2$. For glucose $(180 \ g = 1 \text{ mole})$, $i = 1$. Since both solutes are dissolved in the same amount of solvent ($1000 \ mL \approx 1 \text{ kg}$ of water), their molality $(m)$ is the same. Therefore, $\Delta T_{b} \propto i$. Since $i_{NaCl} > i_{glucose}$, the $NaCl$ solution will show a higher elevation of boiling point.

Class 12 Chemistry Solutions Elevation of boiling point of the solvent

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$58.4 \ g$ of $NaCl$ and $180 \ g$ of glucose were separately dissolved in $1000 \ mL$ of water. Identify the correct statement regarding the elevation of boiling point $(b.p.)$ of the resulting solutions.

WBJEE 2012 All WBJEE

A
$NaCl$ solution will show higher elevation of boiling point
B
Glucose solution will show higher elevation of boiling point
C
Both the solutions will show equal elevation of boiling point
D
The boiling point elevation will be shown by neither of the solutions

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Calculate $\Delta T_b$ of a $0.45 \text{ m}$ solution of a nonvolatile solute in a solvent if the molal elevation constant of the solvent is $3.0 \text{ K kg mol}^{-1}$. (in $\text{ K}$)

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$58.4 \ g$ of $NaCl$ and $180 \ g$ of glucose were separately dissolved in $1000 \ mL$ of water. Identify the correct statement regarding the elevation of boiling point $(b.p.)$ of the resulting solutions.

Similar Questions

For water,$K_b = 0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $200 \ mL$ of water,at what temperature will the resulting solution boil at $1 \ atm$ pressure (in $^oC$)?

Calculate the molal elevation constant $(K_b)$ of a solvent if the boiling point of a $0.12 \ m$ solution is $319.8 \ K$ (Boiling point of pure solvent = $319.5 \ K$).

Calculate $\Delta T_b$ of a $0.45 \text{ m}$ solution of a nonvolatile solute in a solvent if the molal elevation constant of the solvent is $3.0 \text{ K kg mol}^{-1}$. (in $\text{ K}$)

The molal elevation constant is the ratio of the elevation in $B.P.$ to

The boiling point of $0.2 \, mol \, kg^{-1}$ solution of $X$ in water is greater than equimolal solution of $Y$ in water. Which one of the following statements is true in this case?

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